If a saturated solution prepared by dissolving solid BaSO4 in water has [Ba2+]= 1.04*10^5M, what is the value of Ksp for BaSO4?
I'm not to sure what you mean by "the same"
To find the value of the solubility product constant (Ksp) for BaSO4, we need to use the ion concentration values provided.
The balanced equation for the dissociation of BaSO4 is:
BaSO4(s) ⇌ Ba2+(aq) + SO42-(aq)
The molar solubility (s) of BaSO4 is the concentration of Ba2+ and SO42- ions in the saturated solution. Since BaSO4 dissociates in a 1:1 ratio, the concentration of Ba2+ ions in the saturated solution is equal to the molar solubility (s).
Given [Ba2+] = 1.04 * 10^5 M, we can write:
s = [Ba2+] = 1.04 * 10^5 M
Since [SO42-] = s (as the ions are in a 1:1 ratio), we also have [SO42-] = s = 1.04 * 10^5 M.
The solubility product constant (Ksp) expression for BaSO4 is:
Ksp = [Ba2+][SO42-]
Substituting the values we found for [Ba2+] and [SO42-]:
Ksp = (1.04 * 10^5 M) * (1.04 * 10^5 M)
Ksp = 1.08 * 10^10 M^2
Therefore, the value of Ksp for BaSO4 is 1.08 * 10^10 M^2.
To find the value of Ksp (solubility product constant) for BaSO4, we need to use the given concentration of Ba2+ ions and the balanced equation for the dissolution of BaSO4 in water.
The solubility product constant (Ksp) expression for BaSO4 is given by:
Ksp = [Ba2+][SO4^2-]
From the given information, we know that [Ba2+] = 1.04*10^5 M. However, we don't have the concentration of sulfate ions ([SO4^2-]).
To determine the value of [SO4^2-], we need to understand the stoichiometry of the reaction. From the balanced equation for the dissolution of BaSO4:
BaSO4(s) ⇌ Ba2+(aq) + SO4^2-(aq)
We can see that for every BaSO4 molecule that dissolves, one Ba2+ ion and one SO4^2- ion are produced. Therefore, the stoichiometric ratio between Ba2+ and SO4^2- is 1:1.
Since the concentration of Ba2+ is given as 1.04*10^5 M, the concentration of SO4^2- would also be 1.04*10^5 M.
Now, plug these values into the Ksp expression:
Ksp = [Ba2+][SO4^2-]
Ksp = (1.04*10^5 M) * (1.04*10^5 M)
Ksp = 1.0816 * 10^10 M^2
Therefore, the value of Ksp for BaSO4 is 1.0816 * 10^10 M^2.
BaSO4 ==> Ba^+2 + SO4^-2
Ksp + (Ba^+2)(SO4^-2)
Solubility BaSO4 = given.
Then (Ba^+) = same
(SO4^-2) = same.
Solve for Ksp.